Abstract:The sulfur–iodine thermochemical water-splitting cycle is a promising route proposed for hydrogen production. The decomposition temperature remains a challenge in the process. Catalysts, such as Pd supported on Al2O3, are being considered to decrease reaction temperatures. However, little is known regarding the kinetic behavior of such systems. In this work, zinc sulfate thermal decomposition was studied through non-isothermal thermogravimetric analysis to understand the effect of a catalyst within the sulfur–… Show more
“…This suggests that the primarily evolved sulfur compound is SO 3 , likely, from the decomposition of some sulfate groups present on the surface of the kesterite particles. Under the experimental conditions (suitably high temperatures, gas flow), the equilibration of Reaction 5 (vide intra) favors the increased proportions of SO 2 and O 2 , as underlined in many metal sulfate decomposition studies [ 22 , 24 , 26 , 36 ]. In this regard, the evolution of the sulfur oxides taking place up to ca.…”
Section: Resultsmentioning
confidence: 92%
“…Interestingly, that high temperature range is more complex now than under the neutral gas conditions. This could be looked at as the consequence of an efficient oxidation of kesterite towards the individual metal sulfates that decompose shortly afterwards with metal oxide formation via the oxysulfate derivatives at the definite temperatures below 880–900 °C [ 22 , 23 , 24 , 25 , 26 ]. The evolution of SO 3 /SO 2 and its completion by 880–900 °C is the final decomposition event, and no further weight changes take place in any of the nanopowders up to the final temperature of 1000 °C.…”
Section: Resultsmentioning
confidence: 99%
“…The hydrated zinc sulfates ZnSO 4 •nH 2 O, n = 1 to 7, are commonly exemplified by the stable monohydrate ZnSO 4 •H 2 O [ 23 , 24 ]. The latter compound is found by TGA to dehydrate in one step by 250 °C, which is followed by the decomposition of ZnSO 4 , first, at 700–800 °C to oxysulfate ZnO•2ZnSO 4 and, then, at 800–950 °C to ZnO with the release of gaseous SO 3 , as outlined in Reaction 2 [ 24 ]. 3ZnSO 4 •H 2 O → 3ZnSO 4 + ↑3H 2 O → ZnO•2ZnSO 4 + ↑SO 3 → 3ZnO + ↑2SO 3 …”
Thermogravimetry coupled with thermal analysis and quadrupole mass spectroscopy TGA/DTA-QMS were primarily used to assess the oxidation susceptibility of a pool of nanocrystalline powders of the semiconductor kesterite Cu2ZnSnS4 for prospective photovoltaic applications, which were prepared via the mechanochemically assisted synthesis route from two different precursor systems. Each system, as confirmed by XRD patterns, yielded first the cubic polytype of kesterite with defunct semiconductor properties, which, after thermal annealing at 500 °C under neutral gas atmosphere, was converted to the tetragonal semiconductor polytype. The TGA/DTA-QMS determinations up to 1000 °C were carried out under a neutral argon Ar atmosphere and under a dry, oxygen-containing gas mixture of O2:Ar = 1:4 (vol.). The mass spectroscopy data confirmed that under each of the gas atmospheres, a distinctly different, multistep evolution of such oxygen-bearing gaseous compounds as sulfur oxides SO2/SO3, carbon dioxide CO2, and water vapor H2O was taking place. The TGA/DTA changes in correlation with the nature of evolving gases helped in the elucidation of the plausible chemistry linked to kesterite oxidation, both in the stage of nanopowder synthesis/storage at ambient air conditions and during forced oxidation up to 1000 °C in the dry, oxygen-containing gas mixture.
“…This suggests that the primarily evolved sulfur compound is SO 3 , likely, from the decomposition of some sulfate groups present on the surface of the kesterite particles. Under the experimental conditions (suitably high temperatures, gas flow), the equilibration of Reaction 5 (vide intra) favors the increased proportions of SO 2 and O 2 , as underlined in many metal sulfate decomposition studies [ 22 , 24 , 26 , 36 ]. In this regard, the evolution of the sulfur oxides taking place up to ca.…”
Section: Resultsmentioning
confidence: 92%
“…Interestingly, that high temperature range is more complex now than under the neutral gas conditions. This could be looked at as the consequence of an efficient oxidation of kesterite towards the individual metal sulfates that decompose shortly afterwards with metal oxide formation via the oxysulfate derivatives at the definite temperatures below 880–900 °C [ 22 , 23 , 24 , 25 , 26 ]. The evolution of SO 3 /SO 2 and its completion by 880–900 °C is the final decomposition event, and no further weight changes take place in any of the nanopowders up to the final temperature of 1000 °C.…”
Section: Resultsmentioning
confidence: 99%
“…The hydrated zinc sulfates ZnSO 4 •nH 2 O, n = 1 to 7, are commonly exemplified by the stable monohydrate ZnSO 4 •H 2 O [ 23 , 24 ]. The latter compound is found by TGA to dehydrate in one step by 250 °C, which is followed by the decomposition of ZnSO 4 , first, at 700–800 °C to oxysulfate ZnO•2ZnSO 4 and, then, at 800–950 °C to ZnO with the release of gaseous SO 3 , as outlined in Reaction 2 [ 24 ]. 3ZnSO 4 •H 2 O → 3ZnSO 4 + ↑3H 2 O → ZnO•2ZnSO 4 + ↑SO 3 → 3ZnO + ↑2SO 3 …”
Thermogravimetry coupled with thermal analysis and quadrupole mass spectroscopy TGA/DTA-QMS were primarily used to assess the oxidation susceptibility of a pool of nanocrystalline powders of the semiconductor kesterite Cu2ZnSnS4 for prospective photovoltaic applications, which were prepared via the mechanochemically assisted synthesis route from two different precursor systems. Each system, as confirmed by XRD patterns, yielded first the cubic polytype of kesterite with defunct semiconductor properties, which, after thermal annealing at 500 °C under neutral gas atmosphere, was converted to the tetragonal semiconductor polytype. The TGA/DTA-QMS determinations up to 1000 °C were carried out under a neutral argon Ar atmosphere and under a dry, oxygen-containing gas mixture of O2:Ar = 1:4 (vol.). The mass spectroscopy data confirmed that under each of the gas atmospheres, a distinctly different, multistep evolution of such oxygen-bearing gaseous compounds as sulfur oxides SO2/SO3, carbon dioxide CO2, and water vapor H2O was taking place. The TGA/DTA changes in correlation with the nature of evolving gases helped in the elucidation of the plausible chemistry linked to kesterite oxidation, both in the stage of nanopowder synthesis/storage at ambient air conditions and during forced oxidation up to 1000 °C in the dry, oxygen-containing gas mixture.
“…Moreover, a series of high diffraction peaks at 18.5, 26.2, 26.9, 29.2, 34.9, 35.6, 38.5, and 41.0 o assigned to the ZnSO4 were observed for Zn/H-S, indicating the presence of a significant quantity of ZnSO4 on the surface of Zn/H-S [29]. Since the decomposition temperature of ZnSO4 is significantly higher than 550 °C, most of the ZnSO4 on the Zn/H-S is well retained after calcination at 450 °C for 4 h [30]. In contrast, the diffraction peaks at 31.7, 34.4, 36.2, and 47.5 o corresponding to the (100), (002), (101), and (102) lattice planes of ZnO were obviously detected on both Zn/H-Ac and Zn/H-N, suggesting the presence of large-sized and well-crystallized ZnO [31].…”
Section: Structural and Textural Propertiesmentioning
A series of Zn-modified Hβ (Zn/Hβ) catalysts were prepared by using the different zinc precursors such as ZnSO4·7H2O, ZnCl2, C4H6O4Zn·2H2O and Zn(NO3)2·6H2O, and their catalytic performance in the ethanol conversion to propylene reaction was evaluated. Results indicate the amount and strength distribution of acid sites of the Zn/Hβ catalysts were easily tuned by employing different type of zinc precursors. More importantly, when the Zn species were introduced to the Hβ, the propylene yield was significantly enhanced, whereas the yields of the byproducts such as ethylene and C2-C4 alkanes were remarkably suppressed. For the catalyst prepared by using the ZnCl2 precursor (Zn/Hβ-C), a higher propylene yield up to 43.4% was achieved as a result of the moderate amount and distribution of acid sites. The average coking rate of the used Zn/Hβ catalysts strongly depended on the amount of total acid sites, especially the strong acid sites, i.e., the higher the amount of total acid sites of the catalyst, the greater the average coking rate. For the catalyst prepared by using the ZnSO4·7H2O precursor, Zn/Hβ-S exhibited a better stability even after depositing more coke, which is due to the higher amount of strong acid sites.
“…Moreover, a series of diffraction peaks at 18.5, 26.2, 26.9, 29.2, 34.9, 35.6, 38.5 and 41.0 • assigned to the ZnSO 4 (JCPDS 33-1476) were observed for Zn/HBeta-S, indicating the presence of a significant quantity of ZnSO 4 on the surface of Zn/HBeta-S [28]. Since the initial decomposition temperature of ZnSO 4 to ZnO•ZnSO 4 was around 700 • C, most of the ZnSO 4 compound on Zn/HBeta-S was well retained after calcination at 450 • C for 4 h [29]. In contrast, strong diffraction peaks at 31.7, 34.4, 36.2 and 47.5 • corresponding to the (100), (002), ( 101) and (102) lattice planes of ZnO (JCPDS 36-1451) were obviously detected on both Zn/HBeta-Ac and Zn/HBeta-N, suggesting the presence of large-sized and well-crystallized ZnO [30].…”
Section: Structural and Textural Propertiesmentioning
A series of Zn-modified HBeta (Zn/HBeta) catalysts were prepared via the wetness impregnation method with different zinc precursors such as ZnSO4·7H2O, ZnCl2, C4H6O4Zn·2H2O and Zn(NO3)2·6H2O, and their catalytic performance in the conversion of ethanol to propylene reaction was evaluated. Results indicate that the amount and strength distribution of the acid sites of the Zn/HBeta catalysts were easily tuned by employing different types of zinc precursors. More importantly, when the zinc species were introduced to the HBeta, the propylene yield was significantly enhanced, whereas the yields of ethylene and C2–C4 alkanes were remarkably suppressed. For the catalyst prepared by using the ZnCl2 precursor, a higher propylene yield of up to 43.4% for Zn/HBeta-C was achieved as a result of the moderate amount and strength distribution of acid sites. The average coking rate of the used Zn/HBeta catalysts strongly depended on the amount of total acid sites, especially the strong acid sites, i.e., the higher the amount of total acid sites of the catalyst, the greater the average coking rate. For the catalyst prepared by using the ZnSO4·7H2O precursor, Zn/HBeta-S exhibited a better stability even after depositing more coke, which was due to the higher amount of strong acid sites.
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